Question

oxygen is acting as an oxidizing agent in all of the following reactions excepta.\\(\ce{2 c(s) + o2(g) -> 2 co(g)}\\)b.\\(\ce{s(s) + o2(g) -> so2(g)}\\)c.\\(\ce{2 f2(g) + o2(g) -> 2 of2(g)}\\)d.\\(\ce{2 na(s) + o2(g) -> na2o2(s)}\\)e.\\(\ce{2 mg(s) + o2(g) -> 2 mgo(s)}\\)

Explanation:

To determine when oxygen is not an oxidizing agent, we analyze the oxidation state of oxygen in each reaction:

• In options A, B, D, E: Oxygen is reduced (oxidation state decreases from 0 to -2 or -1 in D), so it acts as an oxidizing agent.
• In option C: The reaction is \(2\ F_2(g)+O_2(g)

ightarrow2\ OF_2(g)\). The oxidation state of O in \(OF_2\) is +2 (since F is -1, and \(2\times(-1)+x = 0\) gives \(x = +2\)). Here, oxygen is oxidized (oxidation state increases from 0 to +2), so it acts as a reducing agent, not an oxidizing agent.

Answer:

C. \(2\ F_2(g)+O_2(g)
ightarrow2\ OF_2(g)\)